# Problem: You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.The commercial production of nitric acid involves the following chemical reactions:4 NH3(g) + 5O2(g) → 4 NO(g) + 6 H2O(g)2 NO(g) + O2(g) → 2 NO2(g)3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)In the following redox reaction identify the element undergoing oxidation and the element undergoing reduction.2 NO(g) + O2(g) → 2 NO2(g)

###### FREE Expert Solution

To do so, we need to identify the change in oxidation state for each element in the reaction.

Recall the mnemonic for redox reactions:

Loss Electrons → Oxidation → Reducing Agent

Gain Electrons → Reduction → Oxidizing Agent

Reaction: 2 NO(g) + O2(g) → 2 NO2(g)

Reactants:

For NO:

This is neither a peroxide nor superoxide, which means O.S. of O = –2.

This is also a neutral compound so the total oxidation state is zero.

O.S. of N + O.S. of O = 0

O.S. of N + (–2) = 0

O.S. of N = +2

For O2

This is an atom in its elemental form, which means O.S. of O = 0.

Products: ###### Problem Details

You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.

The commercial production of nitric acid involves the following chemical reactions:

1. 4 NH3(g) + 5O2(g) → 4 NO(g) + 6 H2O(g)
2. 2 NO(g) + O2(g) → 2 NO2(g)
3. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

In the following redox reaction identify the element undergoing oxidation and the element undergoing reduction.

2 NO(g) + O2(g) → 2 NO2(g)